Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their solubility to be more,less, or about the same as in a pure water solution ?Clear AllMore soluble than in purecalcium carbonatewater.Similar solubility as in purebarium fluoridewater.Less soluble than in puresilver bromidewater.

The solubility factor is directly related to ions' concentration. According to Le Chatelier's…

Answered: Each of the insoluble salts below are…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 82CP

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Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 1. 0.1M HCl = 0.1 moles HCl / 1 Liter solution Calculate the moles of OH- in each sampleand record these values in Data Table 1. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 1. Ca(OH)2 Ca2+ + 2OH . Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter . Calculate the Ksp for each trial and theaverage Ksp and record these values inData Table 1. Ksp = [Ca2+][OH-]2 Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.47 25.47 25.47 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.32 28.30 28.43 Mass of Calcium Hydroxide Solution 2.85 2.83 2.96 Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl Volume in Syringe 1.0ml…
Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid-base properties.a. Ag3PO2, Ksp = 1.8x10-18b. CaCO3, Ksp = 8.7x10-9c. Hg2Cl2, Ksp = 1.1x10-18 (Hg2 +2 is the cation in the solution)
Why will silver hydroxide be the least soluble in a solution of higher ph?
Is Ag2SO is added to water ,the salt will be?. Soulable or insoulable? Explain why?
. Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 2. 0.1M HCl = 0.1 moles HCl / 1 Liter solutionCalculate the moles of OH- in each sampleand record these values in Data Table 2. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 2. Ca(OH)2 Ca2+ + 2OH24. Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.37 25.37 25.37 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.18 28.21 28.28 Mass of Calcium Hydroxide Solution Volume of Ca(OH)2 Density = 1.000 g/mL Concentration of HCl (M) Initial HCl volume in Syringe 1.0ml 1.0ml 1.0ml Final HCl volume in Syringe .54ml .58ml .5ml Volume of HCl Delivered .46ml .42ml…
calculate the solubility of each of the following compounds in moles per litre. ignore any acid base properties. a. PbI2, Ksp = 1.4x10^-8 b. CdCO3, Ksp = 5.2x10^-12 c. Sr3(PO4)2, Ksp = 1x10^-31
Which compound in each of the following pairs of compounds is the more soluble one? Solubility Product Constants, , at 25°C Substance Formula Ksp Strontium chromate 3.5x10^-5 Strontium carbonate 9.3x10^-10 Magnesium hydroxide 1.8x10^-11 Copper(II) hydroxide 2.6x10^-19 strontium chromate or strontium carbonate strontium carbonatestrontium chromate magnesium hydroxide or copper(II) hydroxide copper(II) hydroxidemagnesium hydroxide
in a container with HCl solution with volume 400 ml and pH = 1, add the salt of PbCl2. Calculate how many grams of PbCl2 can be dissolved in this container, when we know that Kpt of PbCl2 = 1.6 × 10-⁵?
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction. LiNO₃
Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their solubility to be more, less, or about the same as in a pure water solution ? silver bromide lead hydroxide magnesium carbonate More soluble than in pure water. Similar solubility as in pure water. Less soluble than in pure water.
In which of the following aqueous solutions would you expect AgF to have the lowest solubility? pure water 0.023 M NaF 0.030 M LiF 0.015 M KF 0.0075 M AgNO3
Just fill out Table 1 by writing “+” if the compound is soluble/miscible in the solvent. Otherwise, write “-“. Table 1. Data on the results of solubility tests for C4H6O2. Solubility Test Observations + or - 10% NaOH Clear, colorless solution Litmus paper test (indicate if acidic, basic, or neutral) Blue litmus paper turned red distilled water clear, colorless solution 10% NaHCO3 rapid production of bubbles; clear, colorless solution

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